One mole of ice is converted into water at $1 \ atm$ and $273 \ K$. The entropies of $H_2O_{(s)}$ and $H_2O_{(\ell)}$ are $38.2$ and $60.01 \ J \ mol^{-1} \ K^{-1}$ respectively. The enthalpy change for the conversion is ...... $J \ mol^{-1}$.

Calculate the entropy change when $1 \, \text{mole}$ of ice is converted into water at $0 \, ^\circ\text{C}$. (The enthalpy change for the conversion of ice to liquid at $0 \, ^\circ\text{C}$ is $6.0 \, \text{kJ} \, \text{mol}^{-1}$).

One mole of an ideal gas at $350 \, K$ is in a $2.0 \, L$ vessel with thermally conducting walls,which are in contact with the surroundings. It undergoes isothermal expansion from $2.0 \, L$ to $3.0 \, L$ against a constant external pressure of $4 \, atm$. The change in entropy of the surroundings $(\Delta S_{surr})$ is $...... \, J \, K^{-1}$ (Nearest integer). Given: $R = 8.314 \, J \, K^{-1} \, mol^{-1}$.

For which of the following processes,$\Delta S$ is negative?

For the reaction $H_2O_{(l)} \longrightarrow H_2O_{(g)}$ at $T=100^{\circ} C$ and $P=1 \ atm$,choose the correct option:

Calculate the increase in entropy (approximate) of $3 \ mol$ of hydrogen gas as it changes from $300 \ K$ at $0.1 \ atm$ to $1000 \ K$ at $1 \ atm$ $(C_p = 7 \ cal \ K^{-1} \ mol^{-1})$. $[\log \ 3.33 \approx 0.52, \ \ln \ x = 2.3 \ \log \ x]$ .......$cal \ K^{-1}$